Please help with unanswered parts 132Justify your answer:133134135136137138139140Table 4. HalF Life of CO, at Different Initial PressuresP,co2,Half Life141Bar COz, sinitial-1421.000.70181432.000.69711443.000.69541454.000.6954146147Do the Data from Table 4 support your conclusion about the rate order? Justify your answer:148149150151152153154155156157Compare the results of two methods:158159160161162163164165166 87Part I. Integrated Rate Law89Table 3. Data for the Graphical Analysis9091Time, sP cozInPVPco2co2[CO2] vs Time9211.00E+001.00E +001.20E+009320.2717.63E-01-0.27113571.31E+001.00E+009430.5425.81E-01-0.54227161.72E+008.00E-019540.8134.43E-01-0.8134072.26E+00v=03187x+0.7952R = 0.8819961.0843.38E-01-1.08454372.96E+006.00E-019761.3552.58E-01-1.35567983.88E+004.00E-01981.6261.97E-01-1.6268135.09E +002.00E-01991.8971.50E-01-1.8979476.67E+000.00E+001002.1681.14E-01-2.16908628.75E+00152.5-2.00E-01101102.4398.71E-02-2.44021971.15E+01Time, s102112.7096.65E-02 -2.71035491.50E+01103104Graph 3. P vs t. Show trendline equation, R, give it a proper title.105106107In[CO2] vs Time1/[CO2] vs Time1081.60E+0110911.522,51.40E+01-0.51101.20E+01y=4.7936x - 1.0271R=0.8819111-11.00E+011128.00E+00113-156.00E+00114y=-1.0005x - GE-07R =1-24.00E+001152.00E+00116-2.50.00E+00117as1,5225-3-2.00E+00118Time, sTime, s119120121122Graph 4. InP vst. Show trendline equation, R, give it a proper tiGraph 5. 1P vs t. Show trendline equation, R, give it a proper title123Compare the trendline equations alone with R? for three graphs and make a conclusion about the orderof reaction124125126The order with respect to CO2is:First Order127128The rate constant is (use correct units):1.0005129130The integrated rate law is:In[co2)(co2]1/[CO2]

From part-1 (Integrated rate law), the order of the reaction is calculated as 1st order from the…

Justify your answer: Table 4. Half Life of CO, at Different Initial Pressures Pcoz. Half Life Bar CO2, s 0.7018 0.6971 initial 1.00 2.00 3.00 4.00 0.6954 0.6954 Do the Data from Table 4 support your conclusion about the rate order? Justify your answer: Compare the results of two methods:

Justify your answer: Table 4. Half Life of CO, at Different Initial Pressures Pcoz. Half Life Bar CO2, s 0.7018 0.6971 initial 1.00 2.00 3.00 4.00 0.6954 0.6954 Do the Data from Table 4 support your conclusion about the rate order? Justify your answer: Compare the results of two methods:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Two carbon atoms present in the fossils are used to calculate the age of the fossils bones (and, in…

A: The half life of C-14 is given as 5730 yrs that is, the number of atoms of C-14 present initially…

Q: The decomposition of an organic molecule with the formula C4H6 at 326°C is measured as the decrease…

A: In order to find the rate constant and order of reaction from experimental data, we use the…

Q: 1. The decomposition of Bro- is studied by measuring the concentration of BrO over time, the data…

A: Given, Reaction is of second order. So, first we have to calculate value of rate Constant from…

Q: Data for (A] versus time is given below for the reaction: A → products Time, s [A J. M 0.00 1.00…

A: We will plot the following graphs using EXCEL:

Q: Consider the data presented below. Time 0 40 80 120 160 Moles of 0.100 0.067 0.045 0.030 0.020…

A: First, we will put the values given in the table to calculate the rate constant and to observe that…

Q: The half-life for the radioactive decay of U – 238 is 4.5 billion years and is independent of…

Q: The reaction rate for the decomposition of N2O5 to form NO2 and O2 was studied as a function of…

Q: The decomposition of dinitrogen pentoxide gas at 318.15K is measured as the decrease of N2O5…

A: The decomposition of dinitrogen pentoxide gas, Temperature = 318.15K N2O5 concentration in partial…

Q: The measured C-14 activity of a particular artifact from a cave dwelling in New Mexico is 4.50 dpm.…

A: Given information, The measured C-14 activity of a particular artifact from a cave dwelling in New…

Q: The reaction rate for the decomposition of N2O5 to form NO2 and O2 was studied as a function of…

Q: Consider a radio active material with a half-life time of 30 years following first order reaction.…

Q: Rate (L min1) [H2O2] [KI] 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066

A: The rate law can be written as follows: Rate=KH2O2α×KIβ α is the order of the reaction with respect…

Q: For the decomposition of ammonia on a platinum surface at 856 °C2 NH3N2 + 3 H2the average rate of…

A: The reaction is given below.

Q: Half-life equation for first-order reactions: t1/2=0.683k where t1/2 is the half-life in seconds…

A: The half-life for first order reaction is calculated using the given formula,

Q: he decomposition of N₂O on a platinum surface has a rate constant, k = 1.48 x 10-3 M s-1. 2 N₂O (g)…

Q: By what factor does the fraction of collisions with energy equal to or greater than activation…

Q: 1. Consider the reaction: SO2 + Oa - So: + 02. A rate study of this reaction was conducted at 298 K.…

A: Suppose rate of reaction is given as rate=k×[SO2]a×[O3]b where : a = order with respect to SO2…

Q: The activation energy for a reaction is 50 kJ mol. Determine the effect on the rate constant, i.e.…

A: Given, the activation energy for the reaction (Ea) = 50 KJmol-1 = 50000 Jmol-1 Initial temperature…

Q: Use the data from the experiments below to determine the rate law for the reaction, A + B →…

Q: The decomposition of dinitrogen pentoxide gas at 318.15K is measured as the decrease of N2O5…

A: In order to find the rate constant and order of reaction from experimental data, we use the…

Q: "hat percentage of a material will persist after 60 minutes if it's half-life is 30 minutes? dium 24…

A: Given half life = 30 min We have to find amount of substance left after 60 min

Q: Tjejadioactive djejay follows first-order rate law and for the radioisotope, Sr-90. its half-life…

A: Given, The radioactive decay follows first order rate law, The half life of radioisotope, Sr-90…

Q: A - product Time (s)[A](M) 5.50 1.84 101 The partial data table is from a reaction that was found to…

A: A first order reaction is one in which rate of reaction is directly proportional to the…

Q: 5. Exactly 300 mg of a drug are dissolved into an unknown volume of distilled water. After complete…

A: The time v/s concentration data given is, And the order of the reaction given is 0.

Q: The rate constant (k) for a reaction was measured as a function of temperature. A plot of ln⁡(k)…

Q: The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion…

Q: The rate of reaction between butanone and iodine is studied. In this experiment, butanone is in…

Q: Problem attached

A: First order reaction: Reaction which depend only on concentration of one substrate. Pseudo first…

Q: Consider the following data obtained in a second order reaction: NO2(g) N204(8) Time (min) [NO2], M…

A: Second-order reaction is one whose rate is proportional to the square of the concentration of one…

Q: The radioactive nuclide 63Ni decays by a first-order process via the emission of a beta particle.…

A: Given data: Half life = 160 years Now by using relation between rate constant and half life of 1st…

Q: I was given the below function to describe the half life radioactive decay: N(t)=N0e-kt Where N(t)…

A: half-life(t1/2) of a radioactive decay is the time required to bring down the amount of radioactive…

Q: Question attached

A: Calculate the half-life of the following reaction. X2Y → 2X + Y

Q: The reaction between carbon disulfide and ozone described by the equation Po, (torr) time (s) 1.51…

Q: The decomposition of an organic molecule with the formula C4Hs at 326°C is measured as the decrease…

A: A question based on chemical kinetics, which is to be accomplished.

Q: The activation energy for a reaction is determined to be 314.0 kJ. The rate constant at 23.8°C is…

Q: The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion…

Q: The reaction between the peroxydisulfate ion (S,0,2) and the iodide ion (I) is: S,0g+31, (aq) (aq) +…

A: The rate of the reaction is speed in which the reactants react and convert to form products. The…

Q: Studies of radioactive decay of nuclei show that the decay rate of a radioactive sample is…

A: The decay of a radioactive sample is directly dependent on its amount. Half life of a radioactive…

Q: The radioactive nuclide 63Ni decays by a first-order process via the emission of a beta particle.…

A: Radioactive Decay : It is the process by which an unstable nuclei of an atom loses its energy by…

Q: 11.What is a reaction for which half-life would be applicable? a.14/6C→14/7N+0/−1e…

A: option a first option is the answer half life for radioactive C14 is applicable in this reaction…

Q: Carbon-14 is used to determine the age of biological samples. Carbon-14 decays via a first order…

Q: Complete the following table using the values provided here, and utilize the information to…

A: The expression of activation energy is shown below: ln∆P1∆P2 = EaR1T2-1T1 where; Ea = activation…

Q: The decomposition of H202 in aqueous solution is a first-order process. If [H202lo = 0.882 M and k =…

A: Given, The decomposition of H2O2 in aqueous solution is first order process. Initial…

Q: 3. The decomposition of N₂O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO₂…

Q: Use the data table below to determine the value of the rate law constant for the first order…

A: Rate of a chemical reaction is defined as the speed with which the reaction proceeds. It determines…

Q: In a study of the decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)N20(g) + H20(1)…

A: Since the graph is a straight line having negative slope..this indicates that the order of the…

Q: The half-life period of two samples are 0.1 and 0.4 seconds. Their initialConcentrations are 200 and…

A: The amount of time required by a sample to reduce its initial concentration by half is termed as…

Q: (a) The decomposition of A into products has a value of K as 4.5 × 103 s-1 at 10°C and energy of…

A: Rate of a reaction as well as the rate constant increases with increase in the temperature. The…

Q: 6. Three different sets of data of [A] versus time are given in the table below for the reaction A →…

A: The integrated rate law for zero order reaction is [A] =-kt+[A]o [A] is concentration at time t[A]o…

Q: Calculate the half-life at 100 molecules, 50 molecules and 25 molecules for a 1st order reaction and…

Question

Please help with unanswered parts

132
Justify your answer:
133
134
135
136
137
138
139
140
Table 4. HalF Life of CO, at Different Initial Pressures
P,
co2,
Half Life
141
Bar COz, s
initial-
142
1.00
0.7018
143
2.00
0.6971
144
3.00
0.6954
145
4.00
0.6954
146
147
Do the Data from Table 4 support your conclusion about the rate order? Justify your answer:
148
149
150
151
152
153
154
155
156
157
Compare the results of two methods:
158
159
160
161
162
163
164
165
166

87
Part I. Integrated Rate Law
89
Table 3. Data for the Graphical Analysis
90
91
Time, s
P coz
InP
VP
co2
co2
[CO2] vs Time
92
1
1.00E+00
1.00E +00
1.20E+00
93
2
0.271
7.63E-01
-0.2711357
1.31E+00
1.00E+00
94
3
0.542
5.81E-01
-0.5422716
1.72E+00
8.00E-01
95
4
0.813
4.43E-01
-0.813407
2.26E+00
v=03187x+0.7952
R = 0.8819
96
1.084
3.38E-01
-1.0845437
2.96E+00
6.00E-01
97
6
1.355
2.58E-01
-1.3556798
3.88E+00
4.00E-01
98
1.626
1.97E-01
-1.626813
5.09E +00
2.00E-01
99
1.897
1.50E-01
-1.897947
6.67E+00
0.00E+00
100
2.168
1.14E-01
-2.1690862
8.75E+00
15
2.5
-2.00E-01
101
10
2.439
8.71E-02
-2.4402197
1.15E+01
Time, s
102
11
2.709
6.65E-02 -2.7103549
1.50E+01
103
104
Graph 3. P vs t. Show trendline equation, R, give it a proper title.
105
106
107
In[CO2] vs Time
1/[CO2] vs Time
108
1.60E+01
109
1
1.5
2
2,5
1.40E+01
-0.5
110
1.20E+01
y=4.7936x - 1.0271
R=0.8819
111
-1
1.00E+01
112
8.00E+00
113
-15
6.00E+00
114
y=-1.0005x - GE-07
R =1
-2
4.00E+00
115
2.00E+00
116
-2.5
0.00E+00
117
as
1,5
2
25
-3
-2.00E+00
118
Time, s
Time, s
119
120
121
122
Graph 4. InP vst. Show trendline equation, R, give it a proper ti
Graph 5. 1P vs t. Show trendline equation, R, give it a proper title
123
Compare the trendline equations alone with R? for three graphs and make a conclusion about the order
of reaction
124
125
126
The order with respect to CO2
is:
First Order
127
128
The rate constant is (use correct units):
1.0005
129
130
The integrated rate law is:
In[co2)
(co2]
1/[CO2]

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Given the following data, determine the rate law and calculate K Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4 the units on K are M-2s-1. You should enter the answer without units to 2 sig figs.
For the 2° reaction H2(g) + I2(g) → 2HI(g) at 650 K, the collisional cross section, sigma H2-I2, is 0.36 nm2, the reducedmass is 3.32 × 10−27 kg, and the activation energy is 171 kJ mol−1. Use collision theory to calculate the rateconstant. If the actual value of the rate constant is 8.4 × 10−6 M-1s-1, determine the steric factor for this reaction.
The aqueous-phase decarboxylation of CH2NO2CO2H, CH2NO2CO2H CH3NO2(aq) + CO2(g), is studied at a certain temperature, giving the following data: Time (s) [CH2NO2CO2H] (M) 0.0e+00 0.100 1.0e-01 0.0466 2.0e-01 0.0217 3.0e-01 0.0101 4.0e-01 0.00473 Figure out whether this reaction is first-order or second-order with respect to the concentration of CH2NO2CO2H. Calculate the value of the rate constant. Pick the choice from below which gives the correct reaction order and value of the rate constant for this reaction.
(a) Most commercial heterogeneous catalysts are extremelyfinely divided solid materials. Why is particle sizeimportant? (b) What role does adsorption play in the actionof a heterogeneous catalyst?
A + 3B + 2C --> D + 2E Determine the rate law and rate constant using the experimental data below [A] (M) [B] (M) [C] (M) Rate (M/sec) Exp. 1 0.100 5.00 x 10-4 1.00 x 10-2 0.137 Exp. 2 0.100 1.00 x 10-3 1.00 x 10-2 0.268 Exp. 3 0.200 1.00 x 10-3 1.00 x 10-2 0.542 Exp. 4 0.400 1.00 x 10-3 2.00 x 10-2 1.084
An enzyme-catalyzed reaction is studied in the absence and presence of an inhibitor and the following data was obtained. [S] in mmoles/L Velocity in mmoles/L/min-1 No inhibitor With inhibitor 1.25 1.72 0.98 1.67 2.04 1.17 2.50 2.63 1.47 5.00 3.33 1.96 10.00 4.17 2.38 Calculate the Km of the enzyme in the reaction without inhibitor ________________________ Km’ of the enzyme in the reaction with inhibitor ________________________ Vmax of the uninhibited reaction ________________________ Vmax’ of the inhibited reaction ________________________
The company performs accelerated ageing studies in which a suspension of D is stored at different temperatures. They obtain the degradation rate constants in the table below. Calculate the rate constant for degradation at 25 ºC. (45 % of marks) T / ºC k / d-1 40 0.28 50 0.56
Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/s
Choices for slope: a. -1.35 x 10^4 b. 1.35 x 10^4 c. -1.09 x 10^4 d. 1.09 x 10^4 choices for y intercept: a. -27.8 b. 27.8 c. 37.4 d. -37.4 choices for pearson: a. -0.962 b. -1000 c. -0.982 activation energy a. 9.06 x 10^4 b. 113 c. 90.65 collision frequency factor A a. 1.15 x 10^12 b. 113 c. 90.65
From the equation of the line of best fit for the temperature-rate constant data in Part C, y= -22314x + 25.181 determine the value of Ea in kJ/mol. Include a unit analysis. R is a constant equal to 8.314 J/molK. When you take the natural log of a number, the units disappear.
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?
Ff.22. With explanation...